The Ph of basic buffer mixtures is given by : `Ph=Pk_(a)+`log `(["Base"])/(["Salt"])` whereas Ph of acidic buffer mixtures is given by : Ph =`pK_(a)+"log"(["Salt"])/(["Acid"])`. Addition of little acid or base although shows no appreciable change in Ph for all practical purposes, but sicne the ratio `(["Base"])/(["Salt"])` or `(["Salt"])/(["Acid"])` changes, a slight decrease or increase in pH results.
Calculate the ratio of pH of a solution containing 1 mole of `CH_3COONa` + 1 mole of HCl per litre and of other solution containing 1 mole `CH_3COONa` + 1 mole of acetic acid per litre

Options

A. `1:2`
B. `2:1`
C. `1:3`
D. `3:1`

Explanation

To solve the problem, we need to calculate the pH of two different solutions and then find the ratio of their pH values.

### Step 1: Analyze the first solution (CH₃COONa + HCl)
1. **Identify the components**: The first solution contains 1 mole of sodium acetate (CH₃COONa) and 1 mole of hydrochloric acid (HCl).
2. **Reaction**: The reaction between sodium acetate and hydrochloric acid can be written as:
\[ \text{CH}_3\text{COONa} + \text{HCl} \rightarrow \text{CH}_3\text{COOH} + \text{NaCl} \]
...